{"id":3081,"date":"2023-10-04T10:47:27","date_gmt":"2023-10-04T10:47:27","guid":{"rendered":"http:\/\/localhost\/ecole9ja\/?p=3081"},"modified":"2023-10-04T10:48:28","modified_gmt":"2023-10-04T10:48:28","slug":"week-9-ss2-second-term-chemistry-notes","status":"publish","type":"post","link":"https:\/\/ecolebooks.com\/nigeria\/posts\/week-9-ss2-second-term-chemistry-notes\/","title":{"rendered":"Week 9 &#8211; SS2 Second Term Chemistry Notes"},"content":{"rendered":"<p>\u00a0<strong>WEEK NINE\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0DATE: <\/strong>_________<br \/>\n<strong>TOPIC: COMPOUNDS OF SULPHUR<br \/>\n<\/strong><strong>CONTENT<\/strong><\/p>\n<ul>\n<li>H<sub>2<\/sub>S, SO<sub>2<\/sub> and SO<sub>3<\/sub>: Preparation, Properties and Uses\n<\/li>\n<li>Tetraoxosulphate (VI) acid: Industrial Preparation (Contact Process).\n<\/li>\n<\/ul>\n<p><strong>HYDROGEN SULPHIDE, H<sub>2<\/sub>S<br \/>\n<\/strong>Hydrogen sulphide is found in volcanic gases, sulphur springs, coal gas and natural gas. <\/p>\n<p>\u00a0<strong>LABORATORY PREPARATION<br \/>\n<\/strong>Hydrogen sulphide is prepared in the laboratory by the action of dilute acids on metallic sulphide like Iron (II) sulphide<br \/>\n                2HCl<sub>(aq)<\/sub>    +    FeS<sub>(s)<\/sub> \u2192 FeCl<sub>2(aq)<\/sub> + H<sub>2<\/sub>S<sub>(g)<\/sub><br \/>\n\tThe apparatus used for regular supply of hydrogen sulphide in the laboratory is Kipp&#8217;s apparatus.<strong><br \/>\n\t\t<\/strong><strong>\u00a0\u00a0\u00a0\u00a0<img decoding=\"async\" src=\"https:\/\/ecolebooks.com\/nigeria\/wp-content\/uploads\/9jalessonsimages\/100423_1047_Week9SS2Se1.jpg\" alt=\"\"\/><br \/>\n\t\t<\/strong><br \/>\n\u00a0<strong>PHYSICAL PROPERTIES<br \/>\n<\/strong><\/p>\n<ol>\n<li>\n<div>Hydrogen sulphide is a colourless gas with smell like that of rotten egg.\n<\/div>\n<\/li>\n<\/ol>\n<ol>\n<li>\n<div>It is a very poisonous.\n<\/div>\n<ol>\n<li>\n<div>It is about 1.18 times denser than air.\n<\/div>\n<\/li>\n<\/ol>\n<\/li>\n<li>\n<div>It is moderately soluble in water to form very weak acidic solution.\n<\/div>\n<\/li>\n<li>\n<div>It burns with pale blue flame.\n<\/div>\n<p>\u00a0<\/li>\n<\/ol>\n<p><strong>CHEMICAL PROPERTIES<br \/>\n<\/strong><\/p>\n<ol>\n<li>\n<div>\u00a0\u00a0\u00a0\u00a0As an acid it reacts with alkali to form a normal salt and water \u00a0\u00a0\u00a0\u00a0\n<\/div>\n<\/li>\n<\/ol>\n<p>\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a02NaOH<sub>(aq)<\/sub>     +     H<sub>2<\/sub>S<sub>(g)<\/sub> \u2192 Na<sub>2<\/sub>S<sub>(aq)<\/sub>   +    2H<sub>2<\/sub>O<sub>(l)<\/sub><\/p>\n<ol>\n<li>\n<div>It reacts with excess oxygen to form sulphur (VI) oxide but forms deposit of sulphur with limited oxygen\n<\/div>\n<\/li>\n<\/ol>\n<p>\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a02H<sub>2<\/sub>S<sub>(g)<\/sub>   + 3O<sub>2(g)<\/sub>\u00a0\u00a0\u00a0\u00a0  \u2192     2H<sub>2<\/sub>O<sub>(l)<\/sub> + 2SO<sub>2(g)<\/sub><br \/>\n\t\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a02H<sub>2<\/sub>S<sub>(g)<\/sub>   +  O<sub>2(g)<\/sub>\u00a0\u00a0\u00a0\u00a0   \u2192     2H<sub>2(l)<\/sub> + 2S<sub>(s)<\/sub><\/p>\n<ol>\n<li>\n<div>As a reducing agent, it reacts with many oxidizing agents such as         acidified KMnO4, acidified K<sub>2<\/sub>Cr<sub>2<\/sub>O<sub>7<\/sub>, chlorine gas, FeCl<sub>2<\/sub>, SO<sub>2<\/sub>, H<sub>2<\/sub>SO<sub>4<\/sub> and HNO<sub>3<\/sub>\n\t\t\t<\/div>\n<\/li>\n<\/ol>\n<p>\u00a0<strong>TEST FOR HYDROGEN SULPHIDE<br \/>\n<\/strong>A piece of filter paper is moisten with lead (II) trioxonitrate (V) solution and dropped it into a gas jar of the unknown gas. If the paper turns black, then the gas is H<sub>2<\/sub>S.<\/p>\n<p>\u00a0<strong>EVALUATION<br \/>\n<\/strong><\/p>\n<ol>\n<li>\n<div>Name the reagents used in laboratory preparation of hydrogen sulphide.\n<\/div>\n<\/li>\n<\/ol>\n<ol>\n<li>\n<div>List TWO physical and chemical properties each of hydrogen sulphide.\n<\/div>\n<\/li>\n<\/ol>\n<p>\u00a0<strong>SULPHUR (IV) OXIDE, SO<sub>2<\/sub><br \/>\n\t\t<\/strong><strong>LABORATORY PREPARATION<br \/>\n<\/strong>Sulphur (IV) oxide is prepared in the laboratory by heating sodium or potassium trioxosulphate (IV) with tetraoxosulphate (IV) acid or hydrochloric acid.<br \/>\n         Na<sub>2<\/sub>SO<sub>3(aq)<\/sub>    +   2HCl<sub>(aq)<\/sub>\u00a0\u00a0\u00a0\u00a0\u2192   2NaCl<sub>(aq)<\/sub> + H<sub>2<\/sub>O<sub>(l)<\/sub> + SO<sub>2(g)<\/sub><\/p>\n<p>\u00a0<strong>PHYSICAL PROPERTIES<br \/>\n<\/strong><\/p>\n<ol>\n<li>\n<div>Sulphur (IV) oxide is a colourless poisonous gas with smell like that of burning matches.\n<\/div>\n<ol>\n<li>\n<div>It is very soluble in water.\n<\/div>\n<\/li>\n<li>\n<div>It is about 2.5 times denser than air.\n<\/div>\n<\/li>\n<\/ol>\n<\/li>\n<\/ol>\n<p>\u00a0<strong>CHEMICAL PROPERTIES<br \/>\n<\/strong><\/p>\n<ol>\n<li>\n<div>As an acid, it reacts with alkali to form normal salt of trioxosulphate and water only\n<\/div>\n<p>2NaOH<sub>(aq)<\/sub>    +     SO<sub>2(g)<\/sub> \u2192 Na<sub>2<\/sub>SO<sub>3(aq)<\/sub>  +  H<sub>2<\/sub>O<sub>(l)<\/sub>\n\t\t\t<\/li>\n<li>\n<div>As reducing agent, sulphur (IV) oxide reacts with many oxidizing agents such as acidified KMnO<sub>4<\/sub>; acidified K<sub>2<\/sub>Cr<sub>2<\/sub>O<sub>7;<\/sub> FeCl<sub>3<\/sub>, HNO<sub>3<\/sub>, chlorine gas. It decolorizes acidified purple KMnO<sub>4<\/sub> and turns acidified orange K<sub>2<\/sub>Cr<sub>2<\/sub>O<sub>7<\/sub> to green.\n<\/div>\n<\/li>\n<li>\n<div>It reacts as bleaching agent decolourising dye by its bleaching action. The bleaching action is similar to that of chlorine in that there must be water. But, while chlorine bleaches by oxidation sulphur IV oxide bleaches by reduction.\n<\/div>\n<\/li>\n<li>\n<div>Sulphur (IV) oxide reacts as oxidizing agent in the presence of strong reducing agent such as hydrogen sulphide.\n<\/div>\n<p>2H<sub>2<\/sub>S<sub>(g)<\/sub>   +    SO<sub>2(g)<\/sub> \u2192\u00a0\u00a0\u00a0\u00a02H<sub>2<\/sub>O<sub>(l)<\/sub>    +    3S<sub>(s)<\/sub><br \/>\n\t\t\tC<sub>(s)<\/sub> +   SO<sub>2(g)<\/sub>\u00a0\u00a0\u00a0\u00a0\u2192     CO<sub>2(g)<\/sub>    +    S<sub>(s)<\/sub>\n\t\t\t<\/li>\n<\/ol>\n<p>\u00a0<strong>TEST FOR SO<sub>2<\/sub><br \/>\n\t\t<\/strong><\/p>\n<ol>\n<li>\n<div>If an unknown gas bleaches a coloured flower, SO<sub>2<\/sub> can be suspected\n<\/div>\n<\/li>\n<\/ol>\n<ol>\n<li>\n<div>The unknown gas bubbled through solution of either acidified potassium heptaoxodichromate (VI) or potassium tetraoxomanganate (VII). If orange colour of the acidified K<sub>2<\/sub>Cr<sub>2<\/sub>O<sub>7<\/sub> turn green or the purple colour of the  acidified KMnO<sub>4<\/sub> turns colourless, then the unknown gas is SO<sub>2<\/sub>\n\t\t\t<\/div>\n<\/li>\n<\/ol>\n<p>\u00a0<strong>USES<br \/>\n<\/strong><\/p>\n<ol>\n<li>\n<div>It is used in manufacture of tetraoxosulphate (VI) acid.\n<\/div>\n<\/li>\n<\/ol>\n<ol>\n<li>\n<div>It is used as a germicides and a fumigant especially for destroying termites.\n<\/div>\n<ol>\n<li>\n<div>It is used as bleaching agent for straw, silt and wood.\n<\/div>\n<\/li>\n<li>\n<div>It is used as preservative in some liquid e.g orange juice.\n<\/div>\n<\/li>\n<li>\n<div>Liquid sulphur (IV) oxide is used as refrigerant.\n<\/div>\n<p>\u00a0<strong>EVALUATION<br \/>\n<\/strong><\/li>\n<\/ol>\n<\/li>\n<li>\n<div>Give one method of preparing sulphur (IV) oxide in the laboratory.\n<\/div>\n<\/li>\n<li>\n<div>State THREE physical and chemical properties of sulphur (IV) oxide.\n<\/div>\n<p>\u00a0<\/li>\n<\/ol>\n<p><strong>SULPHUR (VI) OXIDE, SO<sub>3<\/sub><br \/>\n\t\t<\/strong>Sulphur (VI) oxide is prepared by reacting sulphur (IV) oxide and oxygen under special conditions which are:<\/p>\n<ol>\n<li>\n<div>Presence of platinized asbestos or vanadium (V) oxide as catalyst\n<\/div>\n<\/li>\n<li>\n<div>Pressure of 1atm\n<\/div>\n<\/li>\n<\/ol>\n<ol>\n<li>\n<div>Temperature range of 400<sup>o<\/sup>C \u2013 450<sup>o<\/sup>C.\n<\/div>\n<\/li>\n<\/ol>\n<p><img decoding=\"async\" align=\"left\" src=\"https:\/\/ecolebooks.com\/nigeria\/wp-content\/uploads\/9jalessonsimages\/100423_1047_Week9SS2Se2.png\" alt=\"\"\/>\u00a0\u00a0\u00a0\u00a0 2SO<sub>2(g)<\/sub>   +   O<sub>2(g)<\/sub>\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a02SO<sub>3(g)<\/sub><\/p>\n<p>\u00a0<strong>PHYSICAL PROPERTIES OF SO<sub>3<br \/>\n<\/sub><\/strong><\/p>\n<ol>\n<li>\n<div>It exists as white needle-like crystals at room temperature.\n<\/div>\n<\/li>\n<li>\n<div>It has a low boiling point and vapourizes on gentle heating.\n<\/div>\n<\/li>\n<li>\n<div>It dissolves readily in water to give tetraoxosulphate (VI) acid.\n<\/div>\n<\/li>\n<\/ol>\n<p>\u00a0<strong>TRIOXOSULPHATE IV ACID, H<sub>2<\/sub>SO<sub>3<\/sub><br \/>\n\t\t<\/strong>Trioxosulphate (IV) acid is a dibasic acid with a molecular formula H<sub>2<\/sub>SO<sub>3<br \/>\n<\/sub><br \/>\n\u00a0<strong>LABORATORY PREPARATION OF H<sub>2<\/sub>SO<sub>3<\/sub><br \/>\n\t\t<\/strong>It is prepared by the action of dilute hydrochloric acid on heated sodium trioxosulphate (IV) to produce sulphur (IV) oxide, which is then dissolved in water.<br \/>\nNa<sub>2<\/sub>SO<sub>3(s)<\/sub>  +   2HCl<sub>(aq)<\/sub>     \u2192   2NaCl<sub>(aq)<\/sub> + H2O<sub>(l)<\/sub> + S0<sub>2(g)<\/sub><br \/>\n\t<img decoding=\"async\" align=\"left\" src=\"https:\/\/ecolebooks.com\/nigeria\/wp-content\/uploads\/9jalessonsimages\/100423_1047_Week9SS2Se3.png\" alt=\"\"\/>H<sub>2<\/sub>O<sub>(l)<\/sub>  +  SO<sub>2(g)<\/sub>                 H<sub>2<\/sub>SO<sub>3(aq)<\/sub><br \/>\n\tSulphur (IV) Oxide is the acid anhydride of trioxosulphate (IV) acid.<\/p>\n<p>\u00a0<strong>PHYSICAL PROPERTIES OF H<sub>2<\/sub>SO<sub>3<\/sub><br \/>\n\t\t<\/strong><\/p>\n<ol>\n<li>\n<div>It turns blue litmus paper red.\n<\/div>\n<\/li>\n<li>\n<div>It is colourless liquid.\n<\/div>\n<\/li>\n<li>\n<div>It is mixes readily with water.\n<\/div>\n<\/li>\n<\/ol>\n<p>4\u00a0\u00a0\u00a0\u00a0It has an irritating and choking smell.<\/p>\n<p>\u00a0<strong>CHEMICAL PROPERTIES OF H<sub>2<\/sub>SO<sub>3<\/sub><br \/>\n\t\t<\/strong><\/p>\n<ol>\n<li>\n<div>It reacts with alkalis to form salt and water.\n<\/div>\n<p>2NaOH<sub>(aq)<\/sub> + H<sub>2<\/sub>SO<sub>3(aq)<\/sub>    \u2192    Na<sub>2<\/sub>SO<sub>3(aq) <\/sub> + 2H<sub>2<\/sub>O<sub>(l)<\/sub>\n\t\t\t<\/li>\n<li>\n<div>It is oxidized in air to tetraoxosulphate (VI) acid\n<\/div>\n<p>2H<sub>2<\/sub>SO<sub>3(aq) <\/sub> +  O<sub>2(g)<\/sub>   \u2192  2H<sub>2<\/sub>SO<sub>4(aq)<\/sub>\n\t\t\t<\/li>\n<li>\n<div>It reduces oxidizing agent such as potassium tetraoxomanganate (VII) and potassium heptaoxodichromate (VI).\n<\/div>\n<\/li>\n<li>\n<div>It bleaches dyes in the presence of water.\n<\/div>\n<p>\u00a0<\/li>\n<\/ol>\n<p><strong>TEST FOR SO<sub>3<\/sub><sup>2-<\/sup><br \/>\n\t\t<\/strong>Barium chloride solution is added to the solution of the unknown substance. A white<br \/>\nprecipitate soluble in dilute hydrochloric acid confirms the presence of a trioxosulphate (IV)<br \/>\nion.<\/p>\n<p>\u00a0<strong>USES OF H<sub>2<\/sub>SO<sub>3<\/sub><br \/>\n\t\t<\/strong><\/p>\n<ol>\n<li>\n<div>It is used for bleaching straw and other fabrics.\n<\/div>\n<\/li>\n<li>\n<div>It is used as a germicide.\n<\/div>\n<\/li>\n<\/ol>\n<p>\u00a0<strong>EVALUATION<br \/>\n<\/strong><\/p>\n<ol>\n<li>\n<div>Write an equation of reaction for the laboratory preparation of trioxosulphate IV\n<\/div>\n<\/li>\n<li>\n<div>State two physical and two chemical properties of trioxosulphate IV\n<\/div>\n<\/li>\n<\/ol>\n<p>\u00a0<strong>TETRAOXOSULPHATE VI ACID, H<sub>2<\/sub>SO<sub>4<\/sub><br \/>\n\t\t<\/strong>Tetraoxosulphate VI acid is one of the most important chemical compounds known. It is used in almost every manufacturing process; hence it is mostly prepared industrially.<\/p>\n<p>\u00a0<strong>INDUSTRIAL PREPARATION OF H<sub>2<\/sub>SO<sub>4<\/sub><br \/>\n\t\t<\/strong>Industrially, tetraoxosulphate VI acid is manufactured by Contact process. The following steps are involved in Contact process. <\/p>\n<ol>\n<li>\n<div>Burning sulphur in dry air to obtain sulphur (IV) oxide, SO<sub>2<\/sub>\n\t\t\t<\/div>\n<\/li>\n<\/ol>\n<p>\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0S<sub>(s)<\/sub> +  O<sub>2(g)<\/sub>\u00a0\u00a0\u00a0\u00a0\u2192 SO<sub>2<\/sub>(g) <\/p>\n<ol>\n<li>\n<div>The sulphur (IV) oxide produced is mixed with excess air and passed through an electric chamber to remove impurities and dust which may poison the catalyst. The gaseous mixture is then passed through concentrated H<sub>2<\/sub>SO<sub>4<\/sub> to dry it before passing it into the reaction chamber.\n<\/div>\n<\/li>\n<li>\n<div>The dried gaseous mixture is delivered to the contact tower (reaction chamber) where the sulphur (IV) oxide and oxygen combine in the presence of pellets of catalyst, vanadium (V) oxide, V<sub>2<\/sub>O<sub>5<\/sub> to yield sulphur (VI) oxide. The reaction takes place at atmospheric pressure and temperature of 450-500<sup>o<\/sup>C.\n<\/div>\n<\/li>\n<\/ol>\n<p><img decoding=\"async\" align=\"left\" src=\"https:\/\/ecolebooks.com\/nigeria\/wp-content\/uploads\/9jalessonsimages\/100423_1047_Week9SS2Se4.png\" alt=\"\"\/>           2SO<sub>2(g)<\/sub>  +  O<sub>2(g)<\/sub>\u00a0\u00a0\u00a0\u00a0                    2SO<sub>3(g)<\/sub> + heat <\/p>\n<ol>\n<li>\n<div>The sulphur (VI) oxide is cooled and then dissolved in concentrated H<sub>2<\/sub>SO<sub>4<\/sub> to produce a thick liquid called Oleum.\n<\/div>\n<p>         H<sub>2<\/sub>SO<sub>4(aq)<\/sub> +  SO<sub>3(g)  <\/sub>\u2192 H<sub>2<\/sub>S<sub>2<\/sub>O<sub>7(aq) <\/sub>\n\t\t\t<\/li>\n<li>\n<div>The Oleum is then diluted with water appropriately to produce 98% tetraoxosulphate (VI) acid.\n<\/div>\n<\/li>\n<\/ol>\n<p>\u00a0\u00a0\u00a0\u00a0H<sub>2<\/sub>O<sub>(l)<\/sub>  +  H<sub>2<\/sub>S<sub>2<\/sub>O<sub>7(aq)<\/sub>  \u2192  2H<sub>2<\/sub>SO<sub>4(aq)<\/sub><\/p>\n<p>\u00a0<strong>NOTE: <\/strong>Sulphur (VI) oxide is not dissolved directly in water to produce the acid because of the large amount of heat that is evolved in the process. The heat is capable of boiling the acid formed to produce mist of droplets which can spread throughout the factory and cause acid burns.<\/p>\n<p>\u00a0<strong>PHYSICAL PROPERTIES<br \/>\n<\/strong><\/p>\n<ol>\n<li>\n<div>It is a colourless, vicious liquid with density of 1.84gcm<sup>-3<\/sup>\n\t\t\t<\/div>\n<ol>\n<li>\n<div>It is corrosive and cause burns when in contact with the skin.\n<\/div>\n<\/li>\n<li>\n<div>It is highly soluble in water evolving large amount of heat.\n<\/div>\n<\/li>\n<\/ol>\n<\/li>\n<\/ol>\n<p>\u00a0<strong>CHEMICAL PROEPERTIES<br \/>\n<\/strong><\/p>\n<ol>\n<li>\n<div>As an acid, it reacts with metal which are above hydrogen in the electrochemical series to liberate hydrogen gas\n<\/div>\n<\/li>\n<\/ol>\n<p>\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0Zn<sub>(s)<\/sub>  +  H<sub>2<\/sub>SO<sub>4(aq)<\/sub>    \u2192\u00a0\u00a0\u00a0\u00a0 ZnSO<sub>4(aq)<\/sub>  +  H<sub>2(g)<\/sub><\/p>\n<ol>\n<li>\n<div>It reacts with bases to form salts and water\n<\/div>\n<\/li>\n<\/ol>\n<p>\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0MgO<sub>(s)<\/sub>  +\u00a0\u00a0\u00a0\u00a0H<sub>2<\/sub>SO<sub>4(aq)<\/sub> \u2192  MgSO<sub>4(aq)<\/sub>  +  H<sub>2<\/sub>O<sub>(l)<\/sub><\/p>\n<ol>\n<li>\n<div>It reacts with alkali to form normal and acidic salt\n<\/div>\n<\/li>\n<\/ol>\n<p>\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0H<sub>2<\/sub>SO<sub>4(aq)<\/sub>    +    NaOH<sub>(aq)<\/sub>  \u2192 NaHSO<sub>4(aq)<\/sub>  + H<sub>2<\/sub>O<sub>(l)<\/sub><br \/>\n\t\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0H<sub>2<\/sub>SO<sub>4(aq)<\/sub>    +    NaOH<sub>(aq)<\/sub>\u00a0\u00a0\u00a0\u00a0 \u2192 Na<sub>2<\/sub> SO<sub>4(aq)<\/sub> + 2H<sub>2<\/sub>O<sub>(l)<\/sub><\/p>\n<ol>\n<li>\n<div>As an acid, it reacts with trioxocarbonate (IV) to liberate carbon (IV) oxide\n<\/div>\n<\/li>\n<\/ol>\n<p>\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0H<sub>2<\/sub>SO<sub>4(aq)<\/sub>   + CuCO<sub>3(aq)<\/sub>\u00a0\u00a0\u00a0\u00a0\u2192  CuSO<sub>4(aq)<\/sub>  +  H<sub>2<\/sub>O<sub>(l)<\/sub> + CO<sub>2(g)<\/sub><\/p>\n<ol>\n<li>\n<div>As oxidizing agent, concentrated H<sub>2<\/sub>SO<sub>4<\/sub> oxidize metals, non \u2013metals and hydrogen sulphide in the following ways.\n<\/div>\n<\/li>\n<\/ol>\n<p>\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0Zn<sub>(s)<\/sub> +  2H<sub>2<\/sub>SO<sub>4(aq)<\/sub>\u00a0\u00a0\u00a0\u00a0 \u2192  ZnSO<sub>4(aq)<\/sub>  +  2H<sub>2<\/sub>O<sub>(l)<\/sub>\u00a0\u00a0\u00a0\u00a0+  SO<sub>2(g)<\/sub><br \/>\n\t\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0C<sub>(s)<\/sub> + 2H<sub>2<\/sub>SO<sub>4(aq)<\/sub>\u00a0\u00a0\u00a0\u00a0 \u2192  2H<sub>2<\/sub>O<sub>(l)<\/sub>  +  CO<sub>2(g)<\/sub>  + \u00a0\u00a0\u00a0\u00a02SO<sub>2(g)<\/sub><br \/>\n\t\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0H<sub>2<\/sub>SO<sub>4(aq)<\/sub> +  H<sub>2<\/sub>S<sub>(g)<\/sub>\u00a0\u00a0\u00a0\u00a0 \u2192  S<sub>(s)<\/sub>  +  H<sub>2<\/sub>O<sub>(l)<\/sub>  +  SO<sub>2(g)<\/sub><br \/>\n\t6.\u00a0\u00a0\u00a0\u00a0Concentrated tetraoxosulphate (VI) acid is a dehydrating agent, removing water from compounds like sugar, ethanol, methanoic acid and ethanedioic acid<br \/>\nC<sub>12<\/sub>H<sub>22<\/sub>O<sub>11(s)\u00a0\u00a0\u00a0\u00a0<\/sub>    \u2192      12C<sub>(s)      <\/sub>+    11H<sub>2<\/sub>O<sub>(l)<\/sub><br \/>\n\t<sup>sugar \u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0                   charcoal<\/sup><br \/>\n\t7.\u00a0\u00a0\u00a0\u00a0Concentrated tetraoxosulphate (VI) displaces volatile acids from their salts<br \/>\n\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0KCl<sub>(s) <\/sub>+  H<sub>2<\/sub>SO<sub>4(aq)<\/sub>\u00a0\u00a0\u00a0\u00a0\u2192 KHSO<sub>4(aq)<\/sub> + HCl<sub>(g)<br \/>\n<\/sub><br \/>\n\u00a0<strong>TEST FOR SO<sub>4<\/sub><sup>2-<\/sup><br \/>\n\t\t<\/strong>Barium chloride solution is added to the solution of the unknown substance. A white precipitate insoluble in excess dilute hydrochloric acid confirms the presence of a tetraoxosulphate (VI) ion.<\/p>\n<p>\u00a0<strong>USES OF H<sub>2<\/sub>SO<sub>4<\/sub><br \/>\n\t\t<\/strong><\/p>\n<ol>\n<li>\n<div> It is used in production of fertilizers e.g ammonium tetraoxosulphate (VI).\n<\/div>\n<\/li>\n<li>\n<div>It is used in purification of crude oil.\n<\/div>\n<\/li>\n<li>\n<div>It is used as an electrolyte in lead acid accumulator.\n<\/div>\n<\/li>\n<li>\n<div>It is used as drying agent for many gases except NH<sub>3<\/sub> and H<sub>2<\/sub>S gas.\n<\/div>\n<\/li>\n<li>\n<div>It is used to clean metals before electroplating.\n<\/div>\n<p>\u00a0<\/li>\n<\/ol>\n<p><strong>USES OF TETRAOXOSULPHATE (VI) SALTS<br \/>\n<\/strong><\/p>\n<ol>\n<li>\n<div>Ammonium tetraoxosulphate (VI) used as fertilizers\n<\/div>\n<\/li>\n<\/ol>\n<ol>\n<li>\n<div>Sodium tetraoxosulphate (VI) is used in paper manufacture and as a purgative\n<\/div>\n<\/li>\n<li>\n<div>Calcium tetraoxosulphate (VI) is mined as gypsum and when heated forms plaster of Paris used to set broken bones.\n<\/div>\n<\/li>\n<li>\n<div>Aluminum tetraoxosulphate (VI) is used to coagulate precipitate in purification of water\n<\/div>\n<ol>\n<li>\n<div>Iron II tetraoxosulphate (VI) is used to treat anaemia.\n<\/div>\n<p>\u00a0<\/li>\n<\/ol>\n<\/li>\n<\/ol>\n<p><strong>GENERAL EVALUATION\/REVISION<br \/>\n<\/strong><\/p>\n<ol>\n<li>\n<div>Using equations only, outline the steps involve in the Contact process.\n<\/div>\n<\/li>\n<\/ol>\n<ol>\n<li>\n<div>State THREE physical and chemical properties each of tetraoxosulphate (VI) acid\n<\/div>\n<ol>\n<li>\n<div>Give three uses of tetraoxosulphate (VI) salts.\n<\/div>\n<\/li>\n<\/ol>\n<\/li>\n<li>\n<div> A current is passed through three electrolytic cells connected in series containing solutions of silver trioxonitrate (V), copper (II) tetraoxosulphate (VI) and brine respectively. If 12.7g of copper is deposited in the second electrolytic cell, calculate\n<\/div>\n<ol>\n<li>\n<div>the mass of silver deposited in the first cell,\n<\/div>\n<\/li>\n<li>\n<div>the volume of chlorine liberated in the third cell at 17<sup>o<\/sup>C and 800mmHg pressure. [Ag = 108, Cu = 63.5, 1F = 96500C, Molar gas volume at s.t.p = 22.4 dm<sup>3<\/sup>]\n<\/div>\n<\/li>\n<\/ol>\n<\/li>\n<li>\n<div>1.33dm<sup>3<\/sup> of water at 70<sup>o<\/sup>C is saturated by 2.25moles of lead (II) trioxonitrate (V), and 1.33dm<sup>3<\/sup> of water at 18<sup>o<\/sup>C saturated by 0.53mole of the same salt. If 4.50dm<sup>3<\/sup> of the saturated solution are cooled from 70<sup>o<\/sup>C to 18<sup>o<\/sup>C, calculate the amount of solute that will be deposited in\n<\/div>\n<ol>\n<li>\n<div>moles\n<\/div>\n<\/li>\n<li>\n<div>grams  [ Pb = 207, N= =14 O = 16]\n<\/div>\n<p>\u00a0<\/li>\n<\/ol>\n<\/li>\n<\/ol>\n<p><strong>READING ASSIGNMENT<br \/>\n<\/strong>New School Chemistry for Senior Secondary School by O. Y. Ababio (6<sup>th<\/sup> edition), pages 384-396<\/p>\n<p>\u00a0<strong>WEEKEND ASSIGNMENT<br \/>\n<\/strong><strong>SECTION A:  <\/strong>Write the correct option ONLY.<\/p>\n<ol>\n<li>\n<div>The acid anhydride of tetraoxosulphate (VI) acid is a. SO<sub>2<\/sub> b. SO<sub>3<\/sub> c. SO<sub>4<\/sub> d. SO\n<\/div>\n<\/li>\n<li>\n<div>Which of the following compounds gives a white precipitate with acidified barium chloride solution? a. K<sub>2<\/sub>SO<sub>4<\/sub> b. NaNO<sub>3<\/sub> c. KCl d. CaCO<sub>3<\/sub>\n\t\t\t<\/div>\n<\/li>\n<li>\n<div>Why do we acidify the solution used for testing for the presence of S0<sub>4<\/sub><sup>2-<\/sup>a. To prevent the precipitation of any other ion that may be present in the solution. b. To acidify the test solution. c. To increase the rate of the reaction d. The acid acts as catalyst.\n<\/div>\n<\/li>\n<li>\n<div>Which of the following is used as catalyst in the Contact process? a. V<sub>2<\/sub>O<sub>5<\/sub> b. Platinum c. Fe<sub>3<\/sub>O<sub>2<\/sub> d. Nickel\n<\/div>\n<\/li>\n<li>\n<div>What is the colour of tetraoxosulphate VI acid? a. Colourless b. White c. Blue d. Pale white\n<\/div>\n<p>\u00a0<strong>SECTION B<br \/>\n<\/strong><\/li>\n<li>\n<div>Explain why sulphur (VI) oxide is not dissolve directly in water during the Contact process for preparing tetraoxosulphate (VI) acid.\n<\/div>\n<\/li>\n<li>\n<div>Using balanced equations ONLY, describe the stages involved in the manufacture of tetraoxosulphate (VI) acid using the Contact process.\n<\/div>\n<\/li>\n<\/ol>\n","protected":false},"excerpt":{"rendered":"<p>\u00a0WEEK NINE\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0DATE: _________ TOPIC: COMPOUNDS OF SULPHUR CONTENT H2S, SO2 and SO3: Preparation, Properties and&#8230;<\/p>\n","protected":false},"author":1,"featured_media":0,"comment_status":"open","ping_status":"open","sticky":false,"template":"","format":"standard","meta":{"footnotes":""},"categories":[1,248],"tags":[],"class_list":["post-3081","post","type-post","status-publish","format-standard","hentry","category-posts","category-second-term-ss2-chemistry"],"aioseo_notices":[],"_links":{"self":[{"href":"https:\/\/ecolebooks.com\/nigeria\/wp-json\/wp\/v2\/posts\/3081","targetHints":{"allow":["GET"]}}],"collection":[{"href":"https:\/\/ecolebooks.com\/nigeria\/wp-json\/wp\/v2\/posts"}],"about":[{"href":"https:\/\/ecolebooks.com\/nigeria\/wp-json\/wp\/v2\/types\/post"}],"author":[{"embeddable":true,"href":"https:\/\/ecolebooks.com\/nigeria\/wp-json\/wp\/v2\/users\/1"}],"replies":[{"embeddable":true,"href":"https:\/\/ecolebooks.com\/nigeria\/wp-json\/wp\/v2\/comments?post=3081"}],"version-history":[{"count":1,"href":"https:\/\/ecolebooks.com\/nigeria\/wp-json\/wp\/v2\/posts\/3081\/revisions"}],"predecessor-version":[{"id":3082,"href":"https:\/\/ecolebooks.com\/nigeria\/wp-json\/wp\/v2\/posts\/3081\/revisions\/3082"}],"wp:attachment":[{"href":"https:\/\/ecolebooks.com\/nigeria\/wp-json\/wp\/v2\/media?parent=3081"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/ecolebooks.com\/nigeria\/wp-json\/wp\/v2\/categories?post=3081"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/ecolebooks.com\/nigeria\/wp-json\/wp\/v2\/tags?post=3081"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}